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JEE Main & Advanced JEE Main Online Paper (Held on 9 April 2013)

  • question_answer
    The instantaneous rate of disappearance of\[{{\operatorname{MnO}}_{4}}^{-}\operatorname{ion}\] in the following reaction is                 \[4.56\times {{10}^{-3}}\operatorname{M}{{\operatorname{s}}^{-1}}\]                 \[2{{\operatorname{MnO}}_{4}}^{-}+10{{\operatorname{I}}^{-}}+16{{H }^{+}}\to 2{{\operatorname{Mn}}^{2}}^{+}+\] \[5\operatorname{I}+8{{H }_{2}}\operatorname{O}\]                 The rate of appearance \[{{\operatorname{I}}_{2}}\] is :                   JEE Main Online Paper (Held On 09 April 2013)

    A) \[4.56\times {{10}^{-4}}\operatorname{M}{{\operatorname{s}}^{-1}}\]                

    B) \[1.14\times {{10}^{-2}}\operatorname{M}{{\operatorname{s}}^{-1}}\]                

    C) \[1.14\times {{10}^{-3}}\operatorname{M}{{\operatorname{s}}^{-1}}\]                

    D) \[5.7\times {{10}^{-3}}\operatorname{M}{{\operatorname{s}}^{-1}}\]                

    Correct Answer: B

    Solution :

    Rate of reaction \[=-\frac{1}{2}\,[Mn{{O}_{4}}^{-}]=\frac{1}{5}[{{l}_{2}}]\] \[\therefore \]                  Given, \[[MnO_{4}^{-}]=4.56\times {{10}^{-3}}\] \[\because \]     Rate of appearance of \[{{l}_{2}}\] will be \[=\frac{5}{2}\times 4.56\times {{10}^{-3}}\]                 \[=11.4\times {{10}^{-3}}=1.14\times {{10}^{-2}}\,M{{s}^{-1}}\]                


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